Account for the trend in acidity [Fe(OH2)6]2+ < [Fe(OH2)6]3+ <[Al(OH2)6 ]3+ ≈ [Hg(OH2)]2+
and arrange [Na(OH2)6 ], [Sc(OH2)6]3+ , [Mn(OH2)6]2+ , and[Ni(OH2)6]2+ in order of increasing acidity.
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Explanation:
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1. This trend in acidity is due to following reasons :
[Fe(OH)6]2+ < [Fe(OH2)6]3 + ≈ [Hg(OH2)]2+
- It depends on the charge density of central metal and ease with with H2O can be deprotonated.
- Fe2+ complex is weak acid due to its relatively larger ionic radius and low charge
- Fe3+ complex is relatively acidic than Fe2+ due to increase of charge to +3. Thus, it increases the acid strength.
- Al3+ is more acidic than Fe2+ and Fe3+ due to its smaller radius.
2. The order of increasing acidity is -:
[Na(OH2)6]+ < [Mn(OH2)6]2+ < [Ni(OH2)6]2+ < [Sc(OH2)6]3+
- Higher the electronegetivity of central element, higher its tendency to pull electrons towards it. Thus, element with higher electronegetivity is more acidic in nature.
- The order of electronegetivity is :
Sc3+ > Ni2+ > Mn2+ >Na+
- We can see that complex Sc3+ is most acidic and Na+ is least acidic due its electronegetivity. Higher the electronegetivity, more acidic is the compound. Similarly with Mn2+ and Ni2+.
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